Acids, Bases And Salts

Acid is formed by reaction of non-metal oxide with water. This can be illustrated with the help of an example:

CO₂ + H₂O → H₂CO₃

Carbon is a non-metal and thus carbon dioxide is a non-metal oxide. Thus, when a non-metal oxide (CO₂) reacts with water, an acid (carbonic acid) is formed.

When a metal reacts with a base, salt and water are produced. The reaction of the acid with metal oxide is similar to the reaction with a base. This is because the metal oxides are basic in nature.

When strong bases react with some amphoteric metals (which can react with both acids and bases), salt and dihydrogen gas are produced.

Example: 2NaOH + Zn → Na₂ZnO₂ + H₂

Molarity of a solution can be defined as:

If one mole of solute is dissolved in One-litre solution, then the concentration of the solution has 1 molarity. So from the above definition, formula for finding molarity can be written as:

Molarity = no. of moles ÷ volume of solution in litres

For the given question,

No. of moles of HCL = 2

Volume in mL = 500mL

Volume in litres = 500÷1000 = 0.5L

Molarity = 2 ÷ 0.5 = 4M

Concentration of hydronium ions is equivalent to 10^-7M in neutral solutions. Acidic solutions have a greater concentration of

Hydronium ions than Hydroxide ions. Thus acidic solutions have hydronium ion concentration greater than 10^-7 M.

As the concentration of hydroxide ions increases, the basicity also increases and the pOH decreases. If pOH decreases that means pH increases. So, In simple words, the basicity increases with increase in pH. Therefore, The solution having pH = 11.5 is most basic.

The pH scale was presented by S.P.L Sorensen to express the concentration of hydronium ions in a solution conveniently. The range of the pH scale is from 0 to 14 and its limitation is that it is applicable to only aqueous solutions. Thus the statement is incorrect.

To measure the pH of an aqueous solution approximately, the methods used are: pH paper, litmus paper and universal indicator. All these methods give the general idea of the acidity or basicity of the aqueous solution. The pH meter exactly measures the pH of an aqueous solution and returns a numeric value of pH.

As the food enters the stomach, hydrochloric acid is secreted. This decreases the pH in the stomach and becomes helpful in digestion. Sometimes more HCL is secreted to digest certain food products such as eggs, fish etc. This causes the pain in our stomachs and termed as acidity. Basic substances neutralize this acid and reduce the pain. They are known as antacids.

A) solution with pH = 11

pH + pOH = 14

Therefore, pOH = 14-11 = 3

Hence, [OH^-] = 10^-3

B) solution with pH = 8

pOH = 14-8 = 6

Hence, [OH^-] = 10^-6

So the solution with pH = 11 is (10^-3÷10^-6) 1000 times more basic than the solution with pH = 8

Nitric acid completes dissociates in aqueous solution. So it releases more H₃O ⁺. Thus it is a strong acid.

Reaction: HNO₃ + H₂O → H₃O ⁺ + NO₃^-

If 1M Nitric acid is taken then it will completely dissociate in aqueous solution to give 1M H₃O ⁺.

Acetic acid, oxalic acid, and citric acid do not dissociate completely

in aqueous solution, thus they are weak acids.

NH₃ acts as a base because it accepts H ⁺ when dissolved in the water. Ammonia is known as a weak base because its hydroxide (NH₄OH) does not dissociate completely in its aqueous solution. Thus, it is a weak base.

pH = -log₁₀[H ⁺ ]

pOH = -log₁₀[OH^-]

Since the distilled water is neutral,

[H ⁺ ] = [OH^-] = 10^-7

[H ⁺ ] × [OH^-] = 10^-7 × 10^-7

[H ⁺ ] × [OH^-] = 10^-14

Taking negative logarithm on both sides,

-log₁₀[H ⁺ - log₁₀[OH^-] = -log₁₀[10^-14]

pH + pOH = 14

Unit of molecular mass is gram per mole. It means that molecular mass is the mass of one mole. Weight is the mass of some unknown no. of moles.

So by dividing the given weight by molecular mass, we can find the unknown no. of moles.

NH₄ Cl is a salt produced by the neutralization reaction between a strong acid (HCl) and a weak base (NH₄OH). The reaction between them can be represented as follows:

HCL + NH₄OH → NH₄CL + H₂O

Hydrolyses of NH₄CL tales place as follows:

NH₄⁺ + H₂O → NH₃ + H₃O ⁺

Its produces H₃O ⁺ and that’s why the aqueous solutions of salt produced by neutralization of strong acid and a weak base are acidic in nature. Therefore, pH < 7.

The formula to calculate pH is as follows:

pH = -log₁₀[H ⁺ ]

In this question we are already provided with pH, so we have to calculate the concentration of [H ⁺ ] from the above formula.

2 = -log₁₀[H ⁺ ]

So, the [H ⁺ ] = 10^-2 from the above equation. Therefore, 0.01M HCl

will have a pH of 2.

The formula to calculate pOH is as follows:

pOH = -log₁₀[OH^-]

Also, the relation between pH and pOH is: pH + pOH = 14

Therefore, pOH = 14- 8 = 6

Now, using the formula of pOH:

6 = -log₁₀[OH^-]

Therefore, the concentration of hydroxide ions is 1 x 10^-6 M.

As the concentration of H ⁺ ions increase, the acidity increases, and the pH decreases. Thus, we can say that lesser the pH more will be the acidity. Therefore, solution A will have maximum acidity as it has the least pH followed by solution C, followed by solution B and solution D is least acidic as it has a maximum pH of 3.

The given picture explains the concept:

Concentration of hydronium ions is equivalent to 10^-7 M in neutral solutions. For basic solutions the concentration of [H₃O ⁺ ] is less than 10^-7 M. In the above options, only option B has [H₃O ⁺ ] less than 10^-7 M. Thus, option B will be basic.

When the honey bee bites, we feel the pain and irritation because of the presence of acid Melittin in the poison of the honey bee. It contains 26 amino acids. To get relief from the pain, aqueous solutions of basic substances are applied to neutralize the acid.

Arrhenius acid is a hydrogen-containing substance which produces hydrogen ion (H ⁺ ) in its aqueous solution.

Examples of two such acids are Nitric acid and hydrochloric acid.

HNO₃→ H ⁺ + NO₃^-

HCl → H ⁺ + Cl^-

Arrhenius base is hydroxide containing substance and which produces OH- ion in its aqueous solution.

Examples of two such bases are sodium Hydroxide and potassium hydroxide.

NaOH → Na ⁺ + OH^-

KOH → K ⁺ + OH^-

On the reaction of the acid with metal, the products formed are

dihydrogen gas and salt corresponding to the metal.

Acid + Metal → salt of metal + dihydrogen gas

For example:

The amount of solute in relation to the amount of solvent is

called concentration. The concentration of a solution can be expressed in different ways. Four methods of expressing the concentration of a solution are as follows:

•Molarity

•Normality

•Molality

•Percentage proportion

Molarity and normality are more commonly used.

The pH scale was presented by S.P.L Sorensen to express the concentration of hydronium ions in a solution conveniently. The range of the pH scale is from 0 to 14 and it is applicable to only aqueous solutions.

The formula to calculate pH is: pH = -log₁₀[H₃O ⁺ ]

Approximate methods to measure pH are those methods which give the general idea about the basicity and acidity of a given solution.

Two such methods are:

1. Litmus paper: if the colour of litmus paper changes from blue to red it indicates the acidic nature and if the colour of litmus paper changes from red to blue it indicates basic nature. Thus it is an approximate method.

2. pH paper: pH paper is dipped in the solution whose pH is to be determined. There occurs a colour change. By observing the colour of the pH paper, we can get a general idea of the pH of the solution.

Strong acids are those acids which completely dissociate in their aqueous solutions.

Examples:

•Hydrochloric acid

•Nitric acid

Strong bases are those bases which completely dissociate in their aqueous solutions.

Examples:

•Sodium hydroxide

•Potassium hydroxide.

Weak acids are those acids which partially dissociate in their aqueous solutions.

Examples:

•Oxalic acid

•Citric acid

Weak bases are those bases which partially dissociate in their aqueous solutions.

Examples:

•Ammonium hydroxide

•Ammonia

i. Arrhenius acid is a hydrogen-containing substance which produces hydrogen ion (H ⁺ ) in its aqueous solution.

Examples of such acids are Nitric acid and hydrochloric acid.

HNO₃→ H ⁺ + NO₃^-

HCl → H ⁺ + CL^-

Both contain Hydrogenand produce H ⁺

ii. Arrhenius base is hydroxide containing substance and which produces OH- ion in its aqueous solution.

Examples of two such bases are sodium Hydroxide and potassium hydroxide.

NaOH → Na ⁺ + OH^-

KOH → K ⁺ + OH^-

Both contain Hydroxide and produces OH^-

iii. The substances which donate protons [H ⁺ ] to the other substance are called bronsted-lowry acids. The species responsible for acidity is not [H ⁺ ] but [H₃O ⁺ ].

Examples of bronsted-lowry acids are: HCl, HNO₃

iv. Bronsted-lowry base is a substance which accepts proton from other substance. For example ammonia.

When ammonia is dissolved in the water, it accepts a proton from water and thus behaves as a bronsted-lowry base.

v. A system resulting when a solute is dissolved in a solvent is called a solution. The substance which is present in lesser proportion is called solute and the substance which is in present in a larger proportion is known as a solvent.

The amount of solute in relation to the amount of solvent is

called concentration. The concentration of a solution can be expressed in terms of molarity, normality etc.

vi. The pH is defined as the negative logarithm to the base 10 of the concentration of H₃O ⁺ in aqueous solution. In simple words, pH is used to express the hydronium ion concentration in a solution.

Less the pH more will the hydronium ion concentration.

pH = -log₁₀[H₃O ⁺ ]

vii. The pOH is defined as the negative logarithm to the base 10 of the concentration of hydroxide ions in the aqueous solution. In simple words, pOH is used to express the hydroxide ion concentration in a solution. Less the pOH more will be hydroxide ion concentration.

pOH = -log₁₀[OH^-]

viii. Strong acids are those acids which completely ionize or dissociate in their aqueous solutions.

Examples:

•Hydrochloric acid

•Nitric acid

Dissociation of nitric acid: HNO₃→ H ⁺ + NO₃^-

Dissociation of hydrochloric acid: HCl → H ⁺ + CL^-

ix. Weak acids are those acids which partially ionize or dissociate in their aqueous solutions.

Examples:

•Oxalic acid

•Citric acid

x. Strong bases are those bases which completely ionise or dissociate in their aqueous solutions.

Examples:

•Sodium hydroxide

•Potassium hydroxide.

Dissociation of Sodium hydroxide: NaOH → Na ⁺ + OH^-

Dissociation of potassium hydroxide: KOH → K ⁺ + OH^-

xi. Weak bases are those bases which partially ionize or dissociate in their aqueous solutions.

Examples:

•Ammonium hydroxide

•Ammonia

xii. When a reaction takes place between an acid and a base, salt and water are produced. This reaction is called a neutralisation reaction. In this reaction acid and base mutually nullify each other’s properties. An example of such a reaction is:

xiii. The amount of solute in relation to the amount of solvent is

called concentration. The concentration of a solution can be expressed in terms of molarity, normality etc. 1M concentration can be defined as 1 mole of a substance dissolved in 1 litre of a solution.

1. CO₂(g) + H₂O(l) H₂CO₃ (aq)

(carbonic acid)

2. Li₂O(s) + H₂O(l) 2LiOH (aq)

(Lithium hydroxide)

3. H₂SO₄(aq) + 2KOH(aq) K₂SO₄ (aq) + 2H₂0(l)

(potassium (water) Sulphate)

4. 2HCL(aq) + Ca(s) CaCl₂(aq) + H₂(g)

(calcium chloride) (dihydrogen gas)

5 2HNO₃(aq) + CaO(s) Ca(NO₃)₂ (aq) + H₂O(l)

(calcium nitrate) (water)

6. 2HCL(aq) + Na₂CO₃(aq) 2NaCl(aq) + H₂O(l) + CO₂(g)

(sodium chloride) (water) (carbon Dioxide)

7. NaOH(aq) + HCl(aq) NaCl(aq) + H₂O(l)

(sodium chloride) (water)

8. BaCl₂(aq) + H₂SO₄(aq) BaSO₄(s) + HCl(aq)

(barium sulphate) (hydrochloric acid)

9. Ca(OH)₂(aq) + CO₂(g) CaCO₃(s) + H₂O(l)

(calcium carbonate) (water)

10. HNO₃(aq) + NH₄OH(aq) NH₄NO₃(aq) + H₂O(l)

(ammonium nitrate) (water)

11. Na₂SO₄(aq) + Ba(OH)₂(aq) BaSO₄ (s) + 2NaOH(aq)

(barium sulphate) (sodium Hydroxide)

12. AgNO₃(aq) + NaCl(aq) AgCl(s) + NaNO₃(aq)

(silver chloride) (sodium nitrate)

1. Two properties of acids are are as follows:

•The reaction of the acid with metal:

Acids on reaction with metals produce dihydrogen gas and salt corresponding to the metal.

Acid + metal → salt + dihydrogen gas

•The reaction of acid with base:

Salt and water are formed when acids react with bases. This reaction is called a neutralisation reaction.

Acid + Base → salt + water

2. two properties of bases are as follows:

•The reaction of the base with acid:

Salt and water are formed when acids react with bases. This reaction is called a neutralization reaction.

Acid + Base → salt + water

•The reaction of the base with non-metal oxide

This reaction is also similar to the reaction of base with acids. Salt and water are produced in this reaction also.

Base + Non-metal oxide → salt + water

3. two properties of salts are as follows:

•Salt reacts with other acids to form another salt and acid

Salt + acid → other salt + acid

•Salt reacts with another base to form other salt and base.

Salt + base → other salt + base

4. pH = -log₁₀[H ⁺ ]

pOH = -log₁₀[OH^-]

Since the distilled water is neutral,

[H ⁺ ] = [OH^-] = 10^-7

[H ⁺ ] × [OH^-] = 10^-7 × 10^-7

[H ⁺ ] × [OH^-] = 10^-14

Taking negative logarithm on both sides,

-log₁₀[H ⁺ ] - log₁₀[OH^-] = -log₁₀[10^-14]

pH + pOH = 14

5. As the food enters the stomach, hydrochloric acid is secreted. This decreases the pH in the stomach. The pH in the stomach turns between 1 and 3. In the decreased pH, the enzyme pepsin becomes active and helps in the process of digestion.

6. When a reaction takes place between an acid and a base, salt and water are produced. This reaction is called a neutralisation reaction. In this reaction acid and base mutually nullify each other’s properties.

Four such reactions are as follows:

•HCl + NaOH → NaCl + H₂O

•CH₃COOH + NH₄OH → CH₃COONH₄ + H₂O

•HNO₃ + KOH → KNO₃ + H₂O

•H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O

1. [H₃O ⁺ ] = 7.9 x 10^-11 M

The pH can be calculated using the formula:

pH = -log₁₀[H₃O ⁺ ]

putting the value of hydronium ion concentration in above equation, we get:

pH = -log₁₀[7.9 x 10^-11]

pH = 11 - log₁₀[7.9]

using the log table, we get:

pH = 11-0.8976 = 10.10

Since the pH of the solution comes out to be greater than 7, thus the solution is basic in nature.

2. [OH^-] = 0.00424 M

The formula to calculate pOH is:

pOH = -log₁₀[OH^-]

Putting the value of hydroxide ion concentration in above equation:

pOH = -log₁₀[0.00424]

= -log₁₀[4.24 × 10^-3]

= 3 - log₁₀[4.24]

= 3 – 0.6274

= 2.37

Using the relation, pH + pOH = 14

pH = 14- 2.37 = 11.63

3. A) for solution of pH = 11.9, pOH = 2.1

We know that, pOH = -log₁₀[OH^-]

Putting given pOH value in above equation we get:

2.1 = -log₁₀[OH^-]

log₁₀[OH^-] = -2.1

log₁₀[OH^-] = 3 – 2.1 – 3

log₁₀[OH^-] = -3 + 0.9

[OH^-] = antilog = 7.943 × 10^-3 M

B) solution with pH = 8, pOH = 6

6 = - log₁₀[OH^-]

[OH^-] = 10^-6

Dividing the hydroxide ion concentration of s by Ist solution by second solution, we get: (7.943 × 10^-3 ÷ 10^-6 ) = 7943 times.

4. the formula used to find molarity is:

Putting the value of molarity = 0.2 M

Volume in mL = 500 mL

Molar mass = 98 g/mol

Weight = 9.8 g.

So, by adding 9.8 g of H₂SO₄ in the 500mL water, we can prepare its 0.2M solution.

5. the formula used to find molarity is:

Molarity = 0.03 M

Volume in mL = 125 mL

Molar mass of KOH = 56g/ mol

Weight = 0.21 g.

So by adding 0.21 g of KOH in 125 mL water, its 0.03 solution can be prepared.

1. Arrhenius acid is a hydrogen-containing substance which produces hydrogen ion (H ⁺ ) in its aqueous solution.

Examples of such acids are Nitric acid and hydrochloric acid.

HNO₃→ H ⁺ + NO₃^-

HCl → H ⁺ + CL^-

Both contain Hydrogenand produce H ⁺

Arrhenius base is hydroxide containing substance and which produces OH- ion in its aqueous solution.

Examples of two such bases are sodium Hydroxide and potassium hydroxide.

NaOH → Na ⁺ + OH^-

KOH → K ⁺ + OH^-

Both contain Hydroxide and produces OH^-

Limitations of this theory are as follows:

•It is applicable to aqueous solutions only.

•It could not explain the basicity of ammonia as ammonia doesn’t contain hydroxide ion.

•It said that H ⁺ is responsible for the acidity while H ⁺ is very unstable and readily combines with water to form hydronium ion.

2. The substances which donate protons [H ⁺ ] to the other substance are called bronsted-lowry acids. The species responsible for acidity is not [H ⁺ ] but [H₃O ⁺ ].

Examples of bronsted-lowry acids are: HCl, HNO₃

The bronsted-lowry base is a substance which accepts a proton from other substance. For example ammonia.

When ammonia is dissolved in the water, it accepts a proton from water and thus behaves as a bronsted-lowry base.

3. There are two types of methods to measure the pH of a solution. Approximate methods are used to get the general idea about the acidity and basicity of a given solution and exact method is used to know the exact numeric value of pH.

Approximate methods:

1. Litmus paper: if the colour of litmus paper changes from blue to red it indicates the acidic nature and if the colour of litmus paper changes from red to blue it indicates basic nature. Thus, it is an approximate method.

2. pH paper: pH paper is dipped in the solution whose pH is to be determined. There occurs a colour change. By observing the colour of the pH paper, we can get a general idea of the pH of the solution.

Exact method:

1. pH-meter: pH-meter is an instrument used for exact pH value measurement. The pH-meter has two electrodes which are dipped in the solution whose pH is to be determined. The electrodes are attached through a circuit to an indicating box where the pH of the solution is read.

1. In distilled water: [H₃O ⁺ ] × [OH^-] = 10^-14

For solution A, [H₃O ⁺ ] = 10^-14 ÷ [OH^-]

= 10^-14 ÷ (4.3 × 10^-4)

= 2.32 × 10^-11 M

For solution B, [H₃O ⁺ ] = 7.3 × 10^-10 M

•Since the hydronium ion concentration of solution B is more, so its pH will be less.

•The solution having the more pH will be more basic. As solution A will have more pH so it will be more basic.

2. using the relation, pOH + pH = 14

pOH = 14 – pH

= 14 – 9.3

= 4.7

Using, pOH = -log₁₀[OH^-]

4.7 = -log₁₀[OH^-]

log₁₀[OH^-] = -4.7

log₁₀[OH^-] = 5 -4.7 -5

log₁₀[OH^-] = -5 + 0.3

log₁₀[OH^-] = + 0.3

[OH^-] = antilog

[OH^-] = 1.99 × 10^-5

3. molar mass of NaOH = atomic mass of Na + Atomic mass of O + atomic mass of H = 23 + 16 + 1 = 40g/ mol.

Volume of solution = 5 litres

Given weight = 8g

No. of moles = given weight ÷ molar mass

= 8g ÷ 40 g/mol

= 0.2 mole

Molarity = no. of moles ÷ volume in litres

= 0.2 ÷ 5

= 0.04 M

Therefore, the hydroxide ion concentration [OH^-] = 0.04 M

pOH = -log₁₀[OH^-]

pOH = -log₁₀[ 4 × 10^-2]

pOH = 2 -log₁₀[ 4]

pOH = 2- 0.6020 = 1.39

using, pOH + pH = 14

pH = 14 – pOH

pH = 14 - 1.39 = 12.61

1 i.pOH = -log₁₀[OH^-]

pH = -log₁₀[H₃O ⁺ ]

ii. 1.acidic solutions have hydronium ion concentration greater than 10^-7 M and hydroxide ion has a concentration of less than 10^-7 M. Thus the pH of the acidic solution is less than 7.

2. Basic solutions have hydroxide ion concentration greater than 10^-7 M and hydronium ion has a concentration of less than 10^-7 M. Thus the pH is greater than 7.

3. in a neutral solution, the concentration of hydronium ions is equal to that of hydroxide ions which is equal to 10^-7 M. thus the pH is 7.

iii. The limitations of the pH scale are as follows:

•pH scale is applicable to aqueous solutions only.

•pH scale is valid for aqueous solutions having concentration bless than 1 M because its range is 0 to 14.

2. the importance of pH in our daily life is as follows:

•Importance of pH for the existence of living beings:

The various reactions that occur inside living beings require a specific pH range of 7.0 to 7.8. the living beings are not able to survive large changes in pH.

•Importance of pH in digestive systems:

As the food enters the stomach, hydrochloric acid is secreted. This decreases the pH in the stomach. The pH in the stomach turns between 1 and 3. In the decreased pH, the enzyme pepsin becomes active and helps in the process of digestion.

•Importance of pH in stopping the decay of teeth:

When the pH on the inner side of our mouth is less than 5.5 then the tooth decay starts. To prevent the teeth from decaying we use basic toothpastes which neutralise the acid produced inside our mouth.

3. The aqueous solution of the salt produced by neutralization of weak acid and strong base possesses basic nature. This is because the salt produced undergoes hydrolyzes during which it combines with H ⁺ ions from water liberating free hydroxide ions.

For example: Sodium acetate is a salt made by the reaction between strong base NaOH and weak acetic acid.

It undergoes hydrolyzes as follows to liberate hydroxide ions:

An aqueous solution of salt produced by neutralization of a weak base and strong acid possesses acidic nature. This is because such salt undergoes hydrolyzes and produces hydronium ions.

For example ammonium nitrate is made from the reaction between strong acid nitric acid and weak base ammonium hydroxide.

1. pH = 11.65

Therefore, pOH = 14 – 11.65 = 2.35

Using, pOH = -log₁₀[OH^-]

Putting the value of pOH in above equation:

2.35 = -log₁₀[OH^-]

log₁₀[OH^-] = -2.355

log₁₀[OH^-] = 3 -2.35 -3

log₁₀[OH^-] = -3 + 0.65

log₁₀[OH^-] = + 0.65

[OH^-] = antilog

[OH^-] = 4.46 × 10^-3

Now if volume is made 6 times then the concentration will decrease 6 times. So the new concentration is = 4.46× 10^-3÷ 6

= 7.44 × 10^-4

So new pOH = -log₁₀[OH^-]

= -log₁₀[7.44 × 10^-4]

= 4-log₁₀[7.44]

= 4- 0.871

= 3.129

Therefore, new pH is 14 – 3.129 = 10.871

2. A) when concentration is 0.03 M

Using, pH = -log₁₀[H₃O ⁺ ]

= -log₁₀[0.03]

= -log₁₀[3 × 10^-2]

= 2 -log₁₀[3]

= 2 – 0.477

= 1.52

B) When concentration is 0.05 M

Using, pH = -log₁₀[H₃O ⁺ ]

= -log₁₀[0.05]

= -log₁₀[5 × 10^-2]

= 2 -log₁₀[5]

= 2 – 0.699

= 1.30

So the change in pH is = 1.52 – 1.30

= 0.22